Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
![Calculate the ionic radius of the fluoride ion using only the following interionic distances and the radius of
the iodide ion = 219 picometers (pm). RbI, 367 pm;
NaF, 231 pm.
RbBr, 344 pm; KBr, 329 pm; KCl, 314 pm; NaCl, 279 pm;](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F95a4d34c-fd68-437b-a627-0ee0520ede13%2Fa92ff68c-cb2b-4046-b718-96a8129a9bdc%2Fh4tbmcc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Calculate the ionic radius of the fluoride ion using only the following interionic distances and the radius of
the iodide ion = 219 picometers (pm). RbI, 367 pm;
NaF, 231 pm.
RbBr, 344 pm; KBr, 329 pm; KCl, 314 pm; NaCl, 279 pm;
Expert Solution
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Objective
The main objective of the question is to find the ionic radius of the fluoride ion (F-) by using the given radius of the following ions and compounds.
Radius of the iodide ion = 219 pm (picometers)
Radius of RbI = 367 pm
Radius of RbBr = 344 pm
Radius of KBr = 329 pm
Radius of KCl = 314 pm
Radius of NaCl = 279 pm
Radius of NaF = 231 pm
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